Limiting Reagent or Reactant

Q. In the reaction, $2S{O}_2\left(g\right)+O_2\left(g\right)\to 2S{O}_3\left(g\right),$ when $1$ mole of $S{O}_2$ and $1$ mole of $O_2$ are made to react to completion:

1. All the oxygen will be consumed
2. 1.0 mole of $S{O}_3$ will be produced
3. 0.5 mole of $S{O}_2$ is remained
4. All of these

Q.

2.76g of silver carbonate (at mass of Ag = 108) on being heated strongly yields a residue

1. 2.32g

2. 2.16g

3. 2.48g

4. 2.64 g

Q.

How many moles of ${\mathrm{CO}}_2\left(\mathrm{g}\right)$ will be produced when one mole of propane is completely burnt in ${\mathrm{O}}_2$ gas?

Q. How much magnesium sulphide can be obtained from 2.00 g of magnesium and 2.00 g ofSulphur by the reaction, Mg + S→ MgS? Which is the limiting agent? Calculate the amountof one of the reactants which remains unreacted. \lbrack Mg 24, S 32\rbrack

Q.

The reagent that is used up first in a chemical reaction is called:

1. Excess reagent

2. Fastest reagent

3. Smallest reagent

4. Limiting reagent

Q. Aluminium reacts with chlorine gas to form aluminium chloride via the following reaction:
$2Al+3C{l}_2\to 2AlC{l}_3$
How many grams of aluminium chloride could be produced from 34 g of aluminium and 39 g of chlorine gas?

1. 90.53 g
2. 48.86 g
3. 75.23 g
4. 24.36 g

Q. For the combustion of sucrose:
$C_{12}{H}_{22}{O}_{11}+12O_2\to 12C{O}_2+11H_{2}O$
10.0 g of sucrose and 10.0 g of oxygen are made to react. Which of the following reactants will be the limiting reagent and what amount of the excess reactant will be left?

1. Sucrose; 5.02 g
2. Sucrose; 2.53 g
3. Oxygen; 1.09 g
4. Oxygen; 5.02 g

Q. A welding fuel gas contains carbon and hydrogen only. Burning a small sample of it in oxygen gives $3.38g$ carbon dioxide, $0.690g$ of water and no other products. A volume of $10.0L$ (measured at STP) of this welding gas is found to weigh $11.6g$.

Q.

An electric discharge is passes through a mixture containing 50 c.c. of $H_2$ and 50 c.c. of $O_2$. The volume of the gases formed (i) at room temperature and (ii) at ${110}^{\circ }C$ will be:

1. (i) 25 c.c. (ii) 50 c.c

2. (i) 50 c.c. (ii) 75 c.c

3. (i) 25 c.c. (ii) 75 c.c

4. (i) 75 c.c. (ii) 75 c.c

Q. Nitric acid can be neutralized by any base to form a salt and water, as in the following equation: $Mg(OH{)}_2+2HN{O}_3\to Mg(N{O}_3{)}_2+2H_{2}O$
What amount of magnesium nitrate salt will be formed by the reaction of 250 g of magnesium hydroxide and 250 g of nitric acid?

1. 294 g
2. 147 g
3. 636 g
4. 318 g

Q. In the reaction, $2S{O}_2\left(g\right)+O_2\left(g\right)\to 2S{O}_3\left(g\right),$ when $1$ mole of $S{O}_2$ and $1$ mole of $O_2$ are made to react to completion:

1. All the oxygen will be consumed
2. 1.0 mole of $S{O}_3$ will be produced
3. 0.5 mole of $S{O}_2$ is remained
4. All of these

Q. Match the weight of reactants given in column I with weight of products marked (?) given in column II.

	Column I		Column II
a.	$2H_2+O_2\to 2H_{2}O$ $1.0g$ $1.0g$ $?$	p.	0.56 g
b.	$N_2+3H_2\to 2N{H}_3$ $1.0g$ $1.0g$ $?$	q.	1.333 g
c.	$CaC{O}_3\underrightarrow{\Delta }CaO+C{O}_2$ $1.0g$ $?$	r.	1.125 g
d.	$C+2H_2\to C{H}_4$ $1.0g$ $1.0g$ $?$	s.	1.214 g

1. $a\to r,b\to s,c\to p,d\to q$
2. $a\to q,b\to s,c\to p,d\to r$
3. $a\to r,b\to s,c\to q,d\to p$
4. $a\to s,b\to r,c\to p,d\to q$

Q. 51.How much magnesium sulphide can be obtained from 2.00g of magnesium and 2.00g of sulphur by the reaction Mg+s-Mgs? Which is the limiting agent? Calculate the amount of one of the reactants which remains unreached.

Q.

With which of the given pairs $C{O}_2$ resembles

1. HgCl₂, C₂H₂

2. HgCl₂, SnCl₄

3. C₂H₂, NO₂

4. N₂O and NO₂

Q.

Is 400g of oxygen gas enough to burn 20 moles of methane completely?

1. Yes

2. All the above

3. No

4. Insufficient data

Q. Find the moles of HCl gas obtained at STP from the following set of reactions:
$FeC{l}_3+O_2\to F{e}_2{O}_3+C{l}_2\left(g\right)H_2\left(g\right)+C{l}_2\left(g\right)\to 2HCl\left(g\right)$
Starting with 4.56 mol of $FeC{l}_3$ , 33.6 L of $O_2$ at STP and 7 mol of $H_2$ gas.
(Molar mass of Fe = 56 g/mol)

1. 2 mol
2. 4 mol
3. 6 mol
4. 8 mol

Q. The enthalpy of combustion of methane graphite and dihydrogen at $298K$ are $-890.3$ kJ $mo{l}^{-1}$ and $-285.8$ kJ $mo{l}^{-1}$ respectively. Enthalpy of formation of $C{H}_4\left(g\right)$ will be:

1. $-52.27$ $kJ$ $mo{l}^{-1}$
2. $-78.8$ $kJ$ $mo{l}^{-1}$
3. $+74.8$ $kJ$ $mo{l}^{-1}$
4. $+52.26$ $kJ$ $mo{l}^{-1}$

Q. 50.0 kg of $N_2\left(g\right)$ and 10.0 kg of $H_2\left(g\right)$ are mixed to produce $N{H}_3\left(g\right).$ Calculate the mass of $N{H}_3$(g) formed:

1. 40.0 kg
2. 25.0 kg
3. 56.6 kg
4. 14.0 kg

Q. $C{H}_{3}OH\left(l\right)+\frac{3}{2}{O}_2\left(g\right)\to C{O}_2\left(g\right)+2H_{2}O\left(l\right);{△}_r{H}^{\ominus }=-726kJ$

Q. Assertion: When 4 moles of $H_2$ react with 2 moles of $O_2$, then 4 moles of water is formed.
Reason: $O_2$ will act as the limiting reagent

1. Both the assertion and the reason are true, and the reason is the correct explanation of the assertion.
2. Both the assertion and the reason are true, but the reason is not the correct explanation of the assertion.
3. The assertion is true, but the reason is false.
4. Both the assertion and the reason are false statements.

Q. At STP, the volume of ammonia formed using 1 mole of nitrogen and 4 moles of hydrogen on complete reaction is:

1. 22.4 L
2. 44.8 L
3. 67.2 L
4. 11.2 L

Q. If $27\text{g}$ of carbon is mixed with $88\text{g}$ of oxygen and is allowed to burn to produce $C{O}_2$, then:

1. Oxygen is the limiting reagent
2. Volume of $C{O}_2$ gas produced at NTP is $50.4\text{L}$
3. $C$ and $O$ combine in mass ratio $3:8$
4. Volume of unreacted $O_2$ at STP is $11.2\text{L}$

Q. What weight of AgCl will be precipitated when a solution containing 4.77 g of NaCl is added to a solution of 5.77 g of $AgN{O}_3$ ?
(Molar mass of Na = 23 g/mol, Cl = 35.5 g/mol, Ag = 108 g/mol)

1. 3.23 g
2. 5.23 g
3. 3.88 g
4. 4.88 g

Q. If excess water is added into a $100g$ bottle sample labelled as $"112\%H_{2}S{O}_4"$ and is reacted with $5.3g$ $N{a}_{2}C{O}_3$, then find the volume of $C{O}_2$ evolved at STP after the completion of the reaction : [$R=0.0821Latmmol$${}^{-1}{K}^{-1}$]
$H_{2}S{O}_4+N{a}_{2}C{O}_3\to N{a}_{2}S{O}_4+H_{2}O+C{O}_2$

1. 2.46 L
2. 24.6 L
3. 1.12 L
4. 11.2 L

Q. How many moles of $H_2$ will be needed to produce 6 moles of $H_{2}O$ when it reacts with excess of $O_2$ ?

1. 3
2. 4
3. 6
4. 5

Q. 267 g of $AlC{l}_3$ reacts with 120 g of NaOH to give aluminium hydroxide. The produced aluminium hydroxide reacts with 3 mol of $H_{2}S{O}_4$ to give aluminium sulphate. Calculate the moles of aluminium sulphate produced in the reaction.
$AlC{l}_3+3NaOH\to Al(OH{)}_3+3NaCl$
$2Al(OH{)}_3+3H_{2}S{O}_4\to A{l}_2(S{O}_4{)}_3+6H_{2}O$

1. 0.5 mol
2. 0.7 mol
3. 0.4 mol
4. 1.2 mol

Q. Equal volumes of 1M HCl& 1M $H_{2}S{O}_4$ are neutralized by 1M NaOH solution and x & y KJ/equivalent of heat are liberated respectively. Which of the following relations is correct?

1. x = 1/2 y

2. x = 2y

3. x = 4y

4. x = 3y

Q. 0.5 moles of $H_{2}S{O}_4$ is mixed with 0.2 moles of $Ca(OH{)}_2.$ The maximum number of moles of $CaS{O}_4$ formed is:
Reaction: $H_{2}S{O}_4+Ca(OH{)}_2\to CaS{O}_4+2H_{2}O$

1. 0.2 mol
2. 0.5 mol
3. 0.4 mol
4. 1.5 mol

Q. In a series of reactions, 20 mol of L and 10 mol of M were made to react to produce $N$ as a product which was utilized to produce $O$ on reaction with 5 mol of K initially present. Find the moles of $O$ produced.
$4L+3M\to 5N+G$ (Yield = 90 %)
$2N+3K\to 4O+3H$ (Yield = 70 %)

1. 15.86 mol
2. 10.52 mol
3. 6.87 mol
4. 4.67 mol

Q. How many moles of $Zn[Fe{S}_2{]}_2$ can be made from 2 g of $Zn$, 3 g of $Fe$ and 4 g of $S$?
$Zn+2Fe+4S\to Zn[Fe{S}_2{]}_2$
(Given: Molar mass of $Fe$ = 56 g/mol and molar mass of $Zn$ = 65 g/mol)

1. 0.0157 mol
2. 0.0265 mol
3. 0.2650 mol
4. 0.0538 mol